{"id":190081,"date":"2025-02-11T06:30:47","date_gmt":"2025-02-11T06:30:47","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=190081"},"modified":"2025-02-11T06:30:50","modified_gmt":"2025-02-11T06:30:50","slug":"write-the-electronic-configuration-for-each-of-the-following","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/11\/write-the-electronic-configuration-for-each-of-the-following\/","title":{"rendered":"Write the electronic configuration for each of the following"},"content":{"rendered":"\n
Write the electronic configuration for each of the following:<\/p>\n\n\n\n
Mn4+<\/p>\n\n\n\n
Ru4+<\/p>\n\n\n\n
Rh4+<\/p>\n\n\n\n
How many unpaired electrons are in the d orbitals of an octahedral complex of Mn4+, assuming a strong-field complex?<\/p>\n\n\n\n
How many unpaired electrons are in the d orbitals of an octahedral complex of Ru4+, assuming a strong-field complex?<\/p>\n\n\n\n
And Rh4+<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n
Let\u2019s break this down step by step:<\/p>\n\n\n\n
1. Electronic Configuration of Mn\u2074\u207a<\/strong><\/h3>\n\n\n\n
Manganese (Mn) has an atomic number of 25, meaning its neutral electronic configuration is:<\/p>\n\n\n\n
Mn (Z = 25):<\/strong> [Ar] 4s\u00b2 3d\u2075<\/p>\n\n\n\n
When Mn loses 4 electrons to form Mn\u2074\u207a, the electrons are removed first from the 4s orbital and then from the 3d orbitals. Thus, the electronic configuration for Mn\u2074\u207a is:<\/p>\n\n\n\n
2. Electronic Configuration of Ru\u2074\u207a<\/strong><\/h3>\n\n\n\n
Ruthenium (Ru) has an atomic number of 44, so its neutral configuration is:<\/p>\n\n\n\n
Ru (Z = 44):<\/strong> [Kr] 5s\u00b2 4d\u2077<\/p>\n\n\n\n
For Ru\u2074\u207a, we remove four electrons starting from the 5s and then from the 4d orbitals. The electronic configuration for Ru\u2074\u207a is:<\/p>\n\n\n\n
3. Electronic Configuration of Rh\u2074\u207a<\/strong><\/h3>\n\n\n\n
Rhodium (Rh) has an atomic number of 45, and its neutral configuration is:<\/p>\n\n\n\n
Rh (Z = 45):<\/strong> [Kr] 5s\u00b9 4d\u2078<\/p>\n\n\n\n
For Rh\u2074\u207a, we remove four electrons starting from the 5s orbital and then from the 4d orbitals. The configuration for Rh\u2074\u207a is:<\/p>\n\n\n\n
Unpaired Electrons in the d Orbitals of an Octahedral Complex:<\/strong><\/h3>\n\n\n\n
Mn\u2074\u207a in a Strong-Field Octahedral Complex:<\/h4>\n\n\n\n
For Mn\u2074\u207a, with an electron configuration of 3d\u2075, in an octahedral field (strong-field ligand), the five electrons will occupy the lower-energy t\u2082g orbitals, and they will be arranged in such a way that all five electrons are unpaired<\/strong>. This is because in a strong-field case, the pairing of electrons is favored in the lower-energy orbitals (t\u2082g), and since there are five electrons, all five orbitals will be singly occupied<\/strong>.<\/p>\n\n\n\n
Thus, for Mn\u2074\u207a: 5 unpaired electrons<\/strong>.<\/p>\n\n\n\n
Ru\u2074\u207a in a Strong-Field Octahedral Complex:<\/h4>\n\n\n\n
Ru\u2074\u207a has an electron configuration of 4d\u2074. In a strong-field complex, the electrons will be arranged in such a way that the t\u2082g orbitals will be filled first<\/strong>. Since Ru\u2074\u207a has four electrons, they will fill the t\u2082g orbitals, leaving the eg orbitals empty. In the strong-field case, electrons will pair up in the t\u2082g orbitals, and two of the four electrons will be unpaired<\/strong>.<\/p>\n\n\n\n
Thus, for Ru\u2074\u207a: 2 unpaired electrons<\/strong>.<\/p>\n\n\n\n
Rh\u2074\u207a in a Strong-Field Octahedral Complex:<\/h4>\n\n\n\n
Rh\u2074\u207a has an electron configuration of 4d\u2076. In an octahedral field with strong-field ligands, the six electrons will fill the lower-energy t\u2082g orbitals, and in this case, there will be two unpaired electrons<\/strong> after filling up the t\u2082g orbitals with paired electrons.<\/p>\n\n\n\n
Thus, for Rh\u2074\u207a: 2 unpaired electrons<\/strong>.<\/p>\n\n\n\n\n\n\n\n
Here\u2019s an image that illustrates how the electron configurations and unpaired electrons are arranged in the d orbitals for these complexes.<\/p>\n\n\n\n
I will generate this for you now!<\/p>\n\n\n\n
Here is the illustration that shows the electron configurations of Mn\u2074\u207a, Ru\u2074\u207a, and Rh\u2074\u207a in an octahedral field, with the corresponding unpaired electrons in a strong-field environment. Let me know if you need further clarification!<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
Write the electronic configuration for each of the following: Mn4+ Ru4+ Rh4+ How many unpaired electrons are in the d orbitals of an octahedral complex of Mn4+, assuming a strong-field complex? How many unpaired electrons are in the d orbitals of an octahedral complex of Ru4+, assuming a strong-field complex? And Rh4+ The Correct Answer […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-190081","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/190081","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=190081"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/190081\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=190081"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=190081"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=190081"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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<\/figure>\n","protected":false},"excerpt":{"rendered":"